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Ch.9 - Chemical Bonding I: The Lewis Model
All textbooksTro 4th EditionCh.9 - Chemical Bonding I: The Lewis ModelProblem 86b
Chapter 9, Problem 86b

Write an appropriate Lewis structure for each compound. Make certain to distinguish between ionic and molecular compounds. b. ClF5

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Identify the type of compound: ClF5 is a molecular compound because it consists of nonmetals.
Determine the total number of valence electrons: Chlorine (Cl) has 7 valence electrons, and each fluorine (F) also has 7 valence electrons. Therefore, the total is 7 + 5(7) = 42 valence electrons.
Place the least electronegative atom in the center: Chlorine is less electronegative than fluorine, so Cl will be the central atom.
Distribute the electrons: Place a single bond between the central Cl atom and each of the five F atoms. This uses up 10 electrons (5 bonds x 2 electrons per bond).
Distribute the remaining electrons to satisfy the octet rule: Place the remaining 32 electrons as lone pairs on the F atoms (6 electrons per F atom) to complete their octets. The central Cl atom will have 10 electrons, which is acceptable for elements in period 3 or higher.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to indicate bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the behavior of compounds.
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Ionic vs. Molecular Compounds

Ionic compounds are formed through the transfer of electrons from one atom to another, resulting in the formation of charged ions that attract each other. In contrast, molecular compounds consist of atoms that share electrons through covalent bonds. Distinguishing between these types of compounds is crucial for accurately representing their structures and understanding their properties.
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Valence Electrons

Valence electrons are the outermost electrons of an atom and are involved in forming bonds with other atoms. The number of valence electrons determines how an atom can bond and interact with others. For example, in the case of ClF5, understanding the valence electrons of chlorine and fluorine is key to constructing its Lewis structure and determining its molecular geometry.
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Related Practice
Textbook Question

In the Chemistry and the Environment box on free radicals in this chapter, we discussed the importance of the hydroxyl radical in reacting with and eliminating many atmospheric pollutants. However, the hydroxyl radical does not clean up everything. For example, chlorofluorocarbons—which destroy stratospheric ozone—are not attacked by the hydroxyl radical. Consider the hypothetical reaction by which the hydroxyl radical might react with a chlorofluorocarbon: OH(g) + CF2Cl2(g) → HOF(g) + CFCl2(g) Use bond energies to explain why this reaction is improbable. (The C–F bond energy is 552 kJ/mol.)

Textbook Question

Each compound contains both ionic and covalent bonds. Write ionic Lewis structures for each, including the covalent structure for the ion in brackets. Write resonance structures if necessary. a. BaCO3

Textbook Question

Each compound contains both ionic and covalent bonds. Write ionic Lewis structures for each, including the covalent structure for the ion in brackets. Write resonance structures if necessary. b. Ca(OH)2 c. KNO3 d. LiIO